Nernst Equation and Gibbs Energy and Equilibrium Constant

Nernst Equation and Gibbs Energy and Equilibrium Constant

What is the time (in seconds) required to deposit 1.175 g of sodium from molten NaCl using a current of 2 A? (Atomic mas

Na⁺ + e⁻ → Na . 1 mol Na (23.5 g) requires 1F. Moles = (1.175/23.5) = 0.05 mol , Charge = 0.05 × 96500 = 4825 C . t = (Q/I) = (4825/2) = 2412.5 s .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

The resistance of a conductivity cell with 0.01 M NaCl solution is 250 Ω, and its conductivity is 0.0012 S cm⁻¹. What is

kappa = (cell constant/R) , 0.0012 = (cell constant/250) , cell constant = 0.3 cm⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

What is the cell constant of a conductivity cell if the resistance of a 0.01 M KCl solution is 200 Ω and its conductivit

kappa = (cell constant/R) , 0.00141 = (cell constant/200) , cell constant = 0.282 cm⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

What is the cell potential at 298 K for Zn(s) | Zn²⁺(0.01 M) || Cu²⁺(0.1 M) | Cu(s) ? (Given: E°cell = 1.10 V )

Ecell = E°cell - (0.059/2) log ([Zn²⁺]/[Cu²⁺]) = 1.10 - (0.059/2) log (0.01/0.1) = 1.129 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

The standard emf of a cell is 0.96 V, and its equilibrium constant at 298 K is 10³² . How many electrons are transferred

E°cell = (0.059/n) log Kc , 0.96 = (0.059/n) × 32 , n = (1.888/0.96) ≈ 2 .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

A cell has E°cell = 1.10 V and Δr G° = -424600 J/mol at 298 K. What is the number of electrons transferred? (F = 96500 C

Δr G° = -n F E°cell , -424600 = -n × 96500 × 1.10 . n = (424600/96500 × 1.10) = (424600/106150) ≈ 4 .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

A cell Ni(s) | Ni²⁺(0.002 M) || Cl₂(g)(0.5 atm) | Cl⁻(0.05 M) | Pt(s) operates at 298 K. What is the cell potential? (Gi

E°cell = 1.36 - (-0.25) = 1.61 V . Ecell = 1.61 - (0.059/2) log ([Ni²⁺][Cl⁻]²/PCl_₂) = 1.61 - 0.0295 log (0.002 × 0.0025/0.5) = 1.61 + 0.084 = 1.694 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

In a fuel cell operating at 298 K, the cell potential decreases from 1.23 V to 1.17 V when the [H⁺] at the cathode incre

Δ E = -(0.059/n) log ([H⁺]₂/[H⁺]₁) , 1.17 - 1.23 = -0.06 = -(0.059/n) log (1/0.1) . -0.06 = -(0.059/n) × 1 , n = (0.059/0.06) ≈ 1 , but cathode reaction O₂ + 4H⁺ + 4e⁻ , so n = 4 .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

A cell has E°cell = 0.88 V and Δr G° = -169840 J/mol at 298 K. How many electrons are transferred? (F = 96500 C/mol)

Δr G° = -n F E°cell , -169840 = -n × 96500 × 0.88 . n = (169840/96500 × 0.88) = (169840/84920) ≈ 2 .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

The standard Gibbs energy change for a cell reaction is -212.27 kJ/mol, and 2 electrons are transferred. What is the sta

Δr G° = -n F E°cell . -212270 = -2 × 96500 × E°cell , E°cell = 1.1 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

A galvanic cell has E°cell = 0.62 V . If the cell potential becomes 0.68 V at 298 K when [Oxidized] = 0.01 M and [Reduce

Ecell = E°cell - (0.059/n) log ([Ox]/[Red]) , 0.68 = 0.62 - (0.059/n) log (0.01/0.1) . 0.06 = (0.059/n) × 1 , n = (0.059/0.06) ≈ 1 .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

A cell Ni(s) | Ni²⁺(0.001 M) || Cl₂(g)(2 atm) | Cl⁻(0.1 M) | Pt(s) operates at 298 K. What is the cell potential? (Given

E°cell = 1.36 - (-0.25) = 1.61 V . Ecell = 1.61 - (0.059/2) log ([Ni²⁺][Cl⁻]²/PCl_₂) = 1.61 - 0.0295 log (0.001 × 0.01/2) = 1.61 + 0.103 = 1.713 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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